Bohr's Atomic Model 

Bohr's Atomic Model Class 11
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Niels Bohr's model of the atom, proposed in 1913, was a significant contribution to the understanding of atomic structure. It was developed to address the limitations of the earlier Rutherford model, which couldn't explain certain phenomena related to the behavior of electrons.
Bohr's model made several key postulates:
1. Electron Orbits: Electrons orbit the nucleus in fixed, circular paths or orbits at specific distances from the nucleus. Each orbit corresponds to a specific energy level.
2. Quantized Energy Levels: Electrons can only exist in certain orbits with specific, quantized energy levels. Electrons in these orbits do not emit radiation.
3. Energy Absorption and Emission: Electrons can absorb or emit energy only when they move from one allowed orbit to another. When an electron absorbs energy, it moves to a higher energy level, and when it emits energy, it moves to a lower energy level.
4. Angular Momentum Quantization: The angular momentum of an electron in a given orbit is quantized and is an integer multiple of h/2π, where h is Planck's constant.
The Bohr model successfully explained the spectral lines of hydrogen, which was a significant achievement. However, it had limitations. For example, it was only applicable to hydrogen-like atoms with a single electron. It couldn't explain the spectra of atoms with more than one electron and didn't account for the wave-particle duality of electrons, which is a fundamental aspect of quantum mechanics. Later advancements in quantum theory, particularly the development of wave mechanics and quantum mechanics, provided a more comprehensive understanding of atomic structure.
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